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3 years ago

What is the concentration (in ppm) of Mn7+ in a 0.00300 M KMnO4 solution? Note: for dilute aqueous solutions, 1 ppm = 1 mg/L.

Chemistry

1 answer:

aleksklad [387]3 years ago

3 0

We know that there is 1 mole of Mn for every 1 mole of KMnO4, therefore the molarity of Mn is similar with KMnO4:

Mn = 0.00300 M

Molar mass of Mn is 54.94 g / mol. Molarity (M) is moles / L, therefore:

Mn = (0.00300 moles / L) * (54.94 g / mol) * (1000 mg / g)

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Specify which atoms, if any, bear a formal charge in the Lewis structure given and the net charge for the species.

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Answer :

Formal charge on C: (-1)

Formal charge on N: (0)

Net charge: (-1)

Explanation :

First we have to determine the Lewis-dot structure of $CN^-$ .

Lewis-dot structure : It shows the bonding between the atoms of a molecule and it also shows the unpaired electrons present in the molecule.

In the Lewis-dot structure the valance electrons are shown by 'dot'.

The given molecule is, $CN^-$

As we know that carbon has '4' valence electrons and nitrogen has '5' valence electrons.

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According to Lewis-dot structure, there are 6 number of bonding electrons and 4 number of non-bonding electrons.

Now we have to determine the formal charge for each atom.

Formula for formal charge :

$\text{Formal charge}=\text{Valence electrons}-\text{Non-bonding electrons}-\frac{\text{Bonding electrons}}{2}$

$\text{Formal charge on C}=4-2-\frac{6}{2}=-1$

$\text{Formal charge on N}=5-2-\frac{6}{2}=0$

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